What is the effect of stronger charges in ionic compounds, according to Coulomb's Law?
Stronger attraction between ions.
What is the effect of greater distance between ions in ionic compounds, according to Coulomb's Law?
Weaker attraction between ions.
What happens when atoms are too close to each other?
Atoms repel each other due to electron cloud repulsion.
What happens when atoms are too far apart?
There is no interaction, and no bond forms.
What happens when electrons are delocalized in a metallic bond?
Metals become great conductors of heat and electricity.
What happens when electron pairs repel each other, according to VSEPR theory?
It dictates the molecule's geometry.
What are the differences between Interstitial and Substitutional Alloys?
Interstitial Alloys: Smaller atoms fit in between larger atoms. | Substitutional Alloys: Atoms of one element replace atoms of another.
What are the differences between Polar and Nonpolar Covalent Bonds?
Polar Covalent Bond: Unequal sharing of electrons. | Nonpolar Covalent Bond: Equal sharing of electrons.
What are the differences between Formal Charge and Oxidation State?
Formal Charge: A bookkeeping tool for electron distribution. | Oxidation State: A real charge based on electronegativity differences.
Compare and contrast Ionic and Covalent bonds.
Ionic: Transfer of electrons between a metal and nonmetal, forming ions. Strong electrostatic forces. | Covalent: Sharing of electrons between two nonmetals. Weaker intermolecular forces.
Define Ionic Bond.
Bond formed between a metal and a nonmetal through electron transfer, creating ions held together by electrostatic forces.
Define Covalent Bond.
Bond formed when atoms share electrons, typically between two nonmetals.
What is a Cation?
A positively charged ion formed when a metal loses electrons.
What is an Anion?
A negatively charged ion formed when a nonmetal gains electrons.
Define Crystal Lattice.
A 3D arrangement of ions held together by strong electrostatic forces in ionic solids.
Define Metallic Bond.
Bond where electrons are delocalized in an "electron sea", allowing for high conductivity.
Define Resonance.
Occurs when a molecule has multiple valid Lewis structures, and the actual structure is a hybrid of all resonance structures.
Define Formal Charge.
The charge an atom *would* have if all bonding electrons were shared equally. Used to determine the most stable Lewis structure.
Define VSEPR theory.
Theory that predicts the 3D shape of molecules based on electron pair repulsion.
Define Hybridization.
The mixing of atomic orbitals to form new hybrid orbitals, explaining bonding and molecular geometry.
